Chemistry 4.1 Atomic structure and the periodic table NEED TO
... The boiling points of the noble gases increase with increasing relative atomic mass (going down the group). The elements in Group 1 of the periodic table, known as the alkali metals: are metals with low density (the first three elements in the group are less dense than water) react with non-meta ...
... The boiling points of the noble gases increase with increasing relative atomic mass (going down the group). The elements in Group 1 of the periodic table, known as the alkali metals: are metals with low density (the first three elements in the group are less dense than water) react with non-meta ...
8.4-8.6 Electron Configuration, The Explanatory Power of the
... chemical properties is because they have the same number of valence electrons. • Valence electrons, those in the outer most principle energy level, are those that are most important in chemical bonding because they are the most loosely held. • Core electrons are the electrons in lower complete princ ...
... chemical properties is because they have the same number of valence electrons. • Valence electrons, those in the outer most principle energy level, are those that are most important in chemical bonding because they are the most loosely held. • Core electrons are the electrons in lower complete princ ...
The Periodic Table
... and generally shiny; most are solid, ductile, and malleable. ductile: able to be drawn into wires malleable: able to be molded, ...
... and generally shiny; most are solid, ductile, and malleable. ductile: able to be drawn into wires malleable: able to be molded, ...
Atoms, elements and compounds
... All pupils will be able to (Baseline): Recognise that elements are made from only one type of particle known as an atom, which is the smallest part of an element. Most pupils will be able to (Further): Identify the first 20 elements in the periodic table and the elements in Groups 1 and 7 by their n ...
... All pupils will be able to (Baseline): Recognise that elements are made from only one type of particle known as an atom, which is the smallest part of an element. Most pupils will be able to (Further): Identify the first 20 elements in the periodic table and the elements in Groups 1 and 7 by their n ...
Summary of the Periodic Table of Elements: 1. Elements in the same
... c. Atomic size d. Metallic properties 6. Valence electrons are involved in the chemical combining of elements in the forming of molecules. 7. Elements to the left in the periodic table tend to lose electrons. 8. Elements to the right in the periodic table tend to gain electrons. 9. The amount of ene ...
... c. Atomic size d. Metallic properties 6. Valence electrons are involved in the chemical combining of elements in the forming of molecules. 7. Elements to the left in the periodic table tend to lose electrons. 8. Elements to the right in the periodic table tend to gain electrons. 9. The amount of ene ...
STUDY GUIDE CHAPTER 8 TEST AND ELEMENT SYMBOLS
... What element is used to make the most widely used compound in the chemical industry? ...
... What element is used to make the most widely used compound in the chemical industry? ...
chem ch 5 - wbm
... As we move from left to right across the table, we gain protons. There is a greater positive charge on the nucleus. This greater charge pulls harder on the outer electrons, pulling them in ...
... As we move from left to right across the table, we gain protons. There is a greater positive charge on the nucleus. This greater charge pulls harder on the outer electrons, pulling them in ...
Midterm Review
... leaving the salt and still retaining the water or you could evaporate the water, if it was not needed. ...
... leaving the salt and still retaining the water or you could evaporate the water, if it was not needed. ...
Periodic Table Notes Ch. 6 ppt
... radius of an atom when it has become an ion. An ion is an atom or bonded group of atoms that has an overall positive or negative charge. An atom acquires a positive charge by losing electrons or negative charge by gaining electrons!! ...
... radius of an atom when it has become an ion. An ion is an atom or bonded group of atoms that has an overall positive or negative charge. An atom acquires a positive charge by losing electrons or negative charge by gaining electrons!! ...
Midterm Review
... leaving the salt and still retaining the water or you could evaporate the water, if it was not needed. ...
... leaving the salt and still retaining the water or you could evaporate the water, if it was not needed. ...
Atoms and Molecules
... Water is life’s most important compound molecule. Without water, no living creature can survive. ...
... Water is life’s most important compound molecule. Without water, no living creature can survive. ...
The Periodic Table of the Elements
... Properties of Bonds • Ionic compounds are rigid solids with high melting and boiling points. When solid, they are poor conductors of electricity, but when melted are good conductors. Most are Groups 1 and 2 reacting with Groups 16 and 17. • Covalent compounds have low melting and boiling points and ...
... Properties of Bonds • Ionic compounds are rigid solids with high melting and boiling points. When solid, they are poor conductors of electricity, but when melted are good conductors. Most are Groups 1 and 2 reacting with Groups 16 and 17. • Covalent compounds have low melting and boiling points and ...
Chapter 6 notes
... two atoms of the same elements when the atoms are joined. In general, atomic size increases from top to bottom within a _______________ and decreases from left to right across a period. ...
... two atoms of the same elements when the atoms are joined. In general, atomic size increases from top to bottom within a _______________ and decreases from left to right across a period. ...
The History of the Modern Periodic Table
... Valence Electrons • electrons available to be lost, gained, or shared in the formation of chemical compounds • usually in the outermost s and p orbitals for main group elements (Families 1 & 2, and Families 13-18) ...
... Valence Electrons • electrons available to be lost, gained, or shared in the formation of chemical compounds • usually in the outermost s and p orbitals for main group elements (Families 1 & 2, and Families 13-18) ...
THE PERIODIC TABLE Introduction • Dmitri Mendeleev is the father
... • Some metalloids such as silicon, germanium (Ge), and arsenic (As) are semiconductors. • Metalloids have some chemical and physical properties of metals and other properties of nonmetals. 3. Atomic Radius • Atomic radius is the distance between the nucleus and the outermost electron. It affects the ...
... • Some metalloids such as silicon, germanium (Ge), and arsenic (As) are semiconductors. • Metalloids have some chemical and physical properties of metals and other properties of nonmetals. 3. Atomic Radius • Atomic radius is the distance between the nucleus and the outermost electron. It affects the ...
Warm Up - Germainium.net
... • Why does atomic radii (size) decrease across a period? • What happens to ionization energy across a period? • Why does atomic size increase down a group? • What happens to ionization energy down a group? • Hypothesize on the relationship between atomic size and ionization energy. ...
... • Why does atomic radii (size) decrease across a period? • What happens to ionization energy across a period? • Why does atomic size increase down a group? • What happens to ionization energy down a group? • Hypothesize on the relationship between atomic size and ionization energy. ...
Explain what he discovered and draw a diagram of the cathode
... 1.6 – Ionization Energy Questions 1. What does the ionization energy of an element describe? 2. How does nuclear charge contribute to an element’s ionization energy? 3. What is the trend in ionization energy as you go across a period? Down a group? 4. Why do these trends exist? 5. Sort the following ...
... 1.6 – Ionization Energy Questions 1. What does the ionization energy of an element describe? 2. How does nuclear charge contribute to an element’s ionization energy? 3. What is the trend in ionization energy as you go across a period? Down a group? 4. Why do these trends exist? 5. Sort the following ...
Families of Elements
... Elements in group VIIA in the periodic table They are the most chemically active nonmetals They have seven electrons in their outer energy levels All halogens are poisonous in pure form Noble Gases Elements in group VIIIA of the periodic table These elements do not combine chemically exc ...
... Elements in group VIIA in the periodic table They are the most chemically active nonmetals They have seven electrons in their outer energy levels All halogens are poisonous in pure form Noble Gases Elements in group VIIIA of the periodic table These elements do not combine chemically exc ...
CHMB homework Name © Van Der Sluys, 2004 Periodic Table 1
... 20. A colored ion is a (s, p, d, or f) block element. 21. As you go down a group the elements generally become (more / less) metallic. 22. The majority of elements in the periodic table are (metals / nonmetals). 23. Elements in the periodic table are arranged according to their ________________. 24. ...
... 20. A colored ion is a (s, p, d, or f) block element. 21. As you go down a group the elements generally become (more / less) metallic. 22. The majority of elements in the periodic table are (metals / nonmetals). 23. Elements in the periodic table are arranged according to their ________________. 24. ...
Naming Molecular Compounds
... What are binary ionic compounds? What are multivalent metals? What are polyatomic ions? Are ionic compound electrolytes or non-electrolytes? ...
... What are binary ionic compounds? What are multivalent metals? What are polyatomic ions? Are ionic compound electrolytes or non-electrolytes? ...
Unit 3.2 Periodic Table Test
... An electron has the same mass as a proton. An electron has much more mass than a neutron. An electron has about the same mass as a neutron. An electron has much less mass than a proton. An electron has much less mass than a neutron. A proton has more mass than ...
... An electron has the same mass as a proton. An electron has much more mass than a neutron. An electron has about the same mass as a neutron. An electron has much less mass than a proton. An electron has much less mass than a neutron. A proton has more mass than ...
Honors Chapter 6 Powerpoint
... characterized as being different than representative elements because they have electrons in which orbitals? a) p b) d c) s d) f ...
... characterized as being different than representative elements because they have electrons in which orbitals? a) p b) d c) s d) f ...
Noble gas
The noble gases make a group of chemical elements with similar properties. Under standard conditions, they are all odorless, colorless, monatomic gases with very low chemical reactivity. The six noble gases that occur naturally are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and the radioactive radon (Rn).For the first six periods of the periodic table, the noble gases are exactly the members of group 18 of the periodic table.It is possible that due to relativistic effects, the group 14 element flerovium exhibits some noble-gas-like properties, instead of the group 18 element ununoctium. Noble gases are typically highly unreactive except when under particular extreme conditions. The inertness of noble gases makes them very suitable in applications where reactions are not wanted. For example: argon is used in lightbulbs to prevent the hot tungsten filament from oxidizing; also, helium is breathed by deep-sea divers to prevent oxygen and nitrogen toxicity.The properties of the noble gases can be well explained by modern theories of atomic structure: their outer shell of valence electrons is considered to be ""full"", giving them little tendency to participate in chemical reactions, and it has been possible to prepare only a few hundred noble gas compounds. The melting and boiling points for a given noble gas are close together, differing by less than 10 °C (18 °F); that is, they are liquids over only a small temperature range.Neon, argon, krypton, and xenon are obtained from air in an air separation unit using the methods of liquefaction of gases and fractional distillation. Helium is sourced from natural gas fields which have high concentrations of helium in the natural gas, using cryogenic gas separation techniques, and radon is usually isolated from the radioactive decay of dissolved radium, thorium, or uranium compounds (since those compounds give off alpha particles). Noble gases have several important applications in industries such as lighting, welding, and space exploration. A helium-oxygen breathing gas is often used by deep-sea divers at depths of seawater over 55 m (180 ft) to keep the diver from experiencing oxygen toxemia, the lethal effect of high-pressure oxygen, and nitrogen narcosis, the distracting narcotic effect of the nitrogen in air beyond this partial-pressure threshold. After the risks caused by the flammability of hydrogen became apparent, it was replaced with helium in blimps and balloons.